Question
What is hybridization? Describe sp³, sp² and sp hybridization with examples.
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Answer
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1. During estimation of nitrogen present in an organic compound by Kjeldahl's method, the ammonia evolved from 0.5 g of the compound in Kjeldahl's estimation of nitrogen, neutralized 10 mL of $1 M H _2 SO _4$. Find out the percentage of nitrogen in the compound.
2. Explain why $\left( CH _3\right)_3 \stackrel{+}{ C }$ is more stable than $CH _3 \stackrel{+}{ C } H _2$ and $\stackrel{+}{ C } H _3$ is the least stable cation.
→2. Explain why $\left( CH _3\right)_3 \stackrel{+}{ C }$ is more stable than $CH _3 \stackrel{+}{ C } H _2$ and $\stackrel{+}{ C } H _3$ is the least stable cation.
Describe the bulk preparation of dihydrogen by electrolytic method. What is the role of an electrolyte in this process?
What is quantum mechanics? Explain the Schrodinger wave equation for hydrogen.
When metal X is treated with sodium hydroxide, a white precipitate (A) is obtained, which is soluble in excess of NaOH to give soluble complex (B). Compound (A) is soluble in dilute HCl to form compound (C). The compound (A) when heated strongly gives (D), which is used to extract metal. Identify (X), (A), (B), (C) and (D). Write suitable equations to support their identities.
Balance the following reactions by oxidation number method :
(a) $Cl _2 O _7+ H _2 O \longrightarrow ClO _2^{-}+ O _2$ (Basic medium)
(b) $MnO _4^{-}+ H _2 S \longrightarrow Mn ^{2+}+ S + H _2 O$ (Acidic medium)
→(a) $Cl _2 O _7+ H _2 O \longrightarrow ClO _2^{-}+ O _2$ (Basic medium)
(b) $MnO _4^{-}+ H _2 S \longrightarrow Mn ^{2+}+ S + H _2 O$ (Acidic medium)
- Define standard enthalpy of formation. Explain why the enthalpy changes for the reaction given below are not enthalpies of formation of $CaCO_3$ and HBr:
- $\text{CaO(s)}+\text{CO}_2(\text{g})\overrightarrow{\ \ \ \ \ \ \ \ }\ \text{CaCO}_3(\text{s});$ $\Delta_\text{r}\text{H}^\circ=-178.3\text{kJ mol}^{-1}$
- $\text{H}_2(\text{g})+\text{Br}_2(\text{g})\overrightarrow{\ \ \ \ \ \ \ }\ 2\text{HBr(g)};$ $\Delta_\text{r}\text{H}^\circ=-72.8\text{kJ mol}^{-1}$
- Use the bond enthalpies listed below to determine the enthalpy of reaction:
Bond enthalpy $(\Delta\text{H}^\circ)/\text{kJ mol}^{-1}$ of C=O = 741; C-H = 414; H-O = 464; O=O = 498.
Match the ions given in Column I with their nature given in Column II.
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Column I
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Column II
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(i)
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(a)
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Stable due to resonance.
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(ii)
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$\text{F}_3-\text{C}^\oplus$
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(b)
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Destabilised due to inductive effect.
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(iii)
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$\ \ \ \ \ \ \ \ \ \ \ \ \text{CH}_3\\\ \ \ \ \ \ \ \ \ \ \ \ \ |\\\text{CH}_3-\text{C}^\ominus\\\ \ \ \ \ \ \ \ \ \ \ \ \ \ |\\\ \ \ \ \ \ \ \ \ \ \ \ \ \text{CH}_3$
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(c)
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Stabilised by hyperconjugation.
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(iv)
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$\ \ \ \ \ \ \ \ \ \ \ \ \ _\oplus\\\text{CH}_3-\text{CH}-\text{CH}_3$
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(d)
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A secondary carbocation.
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How is dihydrogen obtained from:
- dilute sulphuric acid.
- sodium hydroxide and.
- water.
How would you explain the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium?
Write Lewis structure of the following compounds and show formal charge on each atom. $\mathrm{HNO}_3, \mathrm{NO}_2, \mathrm{H}_2 \mathrm{SO}_4$.
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